An ideal gas expands isothermally and reversi | vedclass

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(C) Given: $V_{1} = 10 \ m^{3}$,$V_{2} = 20 \ m^{3}$,$T = 300 \ K$,$W = -5.187 \ kJ = -5187 \ J$.For an isothermal reversible expansion,the work done

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$3$

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(C) Given: $V_{1} = 10 \ m^{3}$,$V_{2} = 20 \ m^{3}$,$T = 300 \ K$,$W = -5.187 \ kJ = -5187 \ J$.For an isothermal reversible expansion,the work done is given by the formula:$W = -2.303 \ nRT \log_{10} \left(\frac{V_{2}}{V_{1}}ight)$Substituting the values:$-5187 = -2.303 	imes n 	imes 8.314 	imes 300 	imes \log_{10} \left(\frac{20}{10}ight)$$-5187 = -2.303 	imes n 	imes 8.314 	imes 300 	imes 0.3010$$n = \frac{5187}{2.303 	imes 8.314 	imes 300 	imes 0.3010}$$n = \frac{5187}{1729.0} \approx 3 \ mol$.

An ideal gas expands isothermally and reversibly from $10 \ m^{3}$ to $20 \ m^{3}$ at $300 \ K$ performing $5.187 \ kJ$ of work on surroundings. Calculate the number of moles of gas undergoing expansion? $(R = 8.314 \ J \ K^{-1} \ mol^{-1})$

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